Question
In: Chemistry
A hydrocarbon with general formula CxHy was burned completely in air, yielding .18g of water and...
A hydrocarbon with general formula CxHy was burned completely in air, yielding .18g of water and .44 g of carbon dioxide. Which formula could give such data? Please explain step by step process. The answer is C2H4 and molar mass for water is 18. g/mol-1 and CO2 is 44.0 g / mol -1
Solutions
queen_honey_blossom answered 5 months agoRelated Solutions
A hydrocarbon with the general formula CxHy is 92.26% carbon. Experiment shows that 0.311 g hydrocarbon...
A hydrocarbon with the general formula
CxHy is 92.26% carbon. Experiment shows that
0.311 g hydrocarbon fills a 185 mL flask at 88.7 °C with a pressure
of 486 mm Hg.
Calculate the molecular formula for this compound.
When 1.661 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 5.211grams of...
When 1.661 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 5.211grams of CO2 and
2.134 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 42.08 g/mol. Determine the empirical formula
and the molecular formula of the hydrocarbon.
Enter the elements in the order presented in the question.
When 5.895 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.50 grams...
When 5.895 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 18.50 grams of CO2and
7.574 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 42.08 g/mol. Determine the empirical formula
and the molecular formula of the hydrocarbon.
Empirical formula?
Molecular formula?
When 6.597 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.74 grams...
When 6.597 grams of a hydrocarbon, CxHy, were burned in a
combustion analysis apparatus, 21.74 grams of CO2 and 5.935 grams
of H2O were produced. In a separate experiment, the molar mass of
the compound was found to be 40.06 g/mol. Determine the empirical
formula and the molecular formula of the hydrocarbon.
5a. When 4.355 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 14.72...
5a. When 4.355 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 14.72 grams of CO2 and
3.014 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 26.04 g/mol. Determine the empirical formula
and the molecular formula of the hydrocarbon.
Enter the elements in the order presented in the
question.
empirical formula =
molecular formula =
5b.
A 12.57 gram sample of an organic compound
containing C,...
When 6.104 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 19.15 grams...
When 6.104 grams of a hydrocarbon, CxHy, were burned in a
combustion analysis apparatus, 19.15 grams of CO2 and 7.842 grams
of H2O were produced. In a separate experiment, the molar mass of
the compound was found to be 28.05 g/mol. Determine the empirical
formula and the molecular formula of the hydrocarbon.
A 7.797 gram sample of an organic compound
containing C, H and O is analyzed by combustion analysis and
7.623 grams of CO2 and
1.561 grams of H2O...
When 6.104 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 19.15 grams...
When 6.104 grams of a hydrocarbon, CxHy, were burned in a
combustion analysis apparatus, 19.15 grams of CO2 and 7.842 grams
of H2O were produced. In a separate experiment, the molar mass of
the compound was found to be 28.05 g/mol. Determine the empirical
formula and the molecular formula of the hydrocarbon.
A 7.797 gram sample of an organic compound containing C, H and O
is analyzed by combustion analysis and 7.623 grams of CO2 and 1.561
grams of H2O...
when 4.027 grams hydrocarbon, CxHy, we're burned in a combustion analysis apparatus, 12.64 grams of CO2...
when 4.027 grams hydrocarbon, CxHy, we're burned in a
combustion analysis apparatus, 12.64 grams of CO2 and 5.174 grams
H2O we're produced.
I need empirical and molecular formulas
1)When 5.352 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.38 grams...
1)When 5.352 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 18.38 grams of CO2 and
3.010grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 128.2 g/mol. Determine the empirical formula
and the molecular formula of the hydrocarbon.
2)When 4.948 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 16.72 grams of CO2 and
3.424grams of H2O were produced.
In a separate experiment, the...
A mixture of saturated hydrocarbon and N2 us burned in excess air supplied at 25°C, 740...
A mixture of saturated hydrocarbon and N2 us burned in excess
air supplied at 25°C, 740 torrs with 90% RH. An orsat analysis of
the stack gas shows 7.6% CO2, 2.28% CO, 1.14% H2, 6.03% O2 and
82.95% N2. With a dew point of 53.46°C. The stack gases leave at
300°C, 765 mmHg with a volume ratio of 2.049 m3 wet stack gas/m3
wet air.
a. The formula of hydrocarbon is?
b. Mole % analysis of the fuel
c. %...
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